At 700 K,K_p for the following equilibrium is 5.6 × 10^-3. 2HgO(s) 2Hg(l) + O₂(g)
Suppose 43.1 g of mercury(II) oxide is placed in a sealed 4.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol) )

Question

At 700 K,K_p for the following equilibrium is 5.6 × 10^-3. 2HgO(s) At 700 K,Kp for the following equilibrium is 5.6 × 10-3. 2HgO(s) 2Hg(l) + O2(g) Suppose 43.1 g of mercury(II) oxide is placed in a sealed 4.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol) ) A) 0.074 atm B) 0.0056 atm C) 2.8 atm D) 14 atm E) 1.4 atm

At 700 K,K<sub>p</sub> for the following equilibrium is 5.6 × 10<sup>-3</sup>. 2HgO(s) 2Hg(l) + O<sub>2</sub>(g) Suppose 43.1 g of mercury(II) oxide is placed in a sealed 4.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol) ) A) 0.074 atm B) 0.0056 atm C) 2.8 atm D) 14 atm E) 1.4 atm

2Hg(l) + O₂(g)
Suppose 43.1 g of mercury(II) oxide is placed in a sealed 4.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol) )

Quizplus · Accepted Answer

The Answer of At 700 K,K_p for the following equilibrium is 5.6 × 10^-3. 2HgO(s) 2Hg(l)+ O₂(g) Suppose 43.1 g of mercury(II)oxide is placed in a sealed 4.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol))

At 700 K,Kp for the Following Equilibrium Is 5

At 700 K,K_p for the Following Equilibrium Is 5